-
15
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
Denisov Evgeny and Denisova Taisa Institute of Problems of
Chemical Physics RAS
Russia
1. Introduction
The bond dissociation energy is very important characteristic of
molecule that usually refers to standard thermodynamic state in gas
phase (298 K, pressure 1 atm). When these thermodynamic quantities
are known they become an invaluable tool for calculation of
activation energies and rate constants of homolytic reactions.
Phenols are widely used as antioxidants for stabilization of
organic compounds and materials. Many organic compounds are
oxidized by oxygen due to contact with air. Phenols are used for
stabilization of variety organic products such as polyolefins,
polystyrene, and rubbers (Hamid, 2000; Scott, 1980; Pospisil &
Klemchuk, 1990; Scott, 1993), monomers (Mogilevich & Pliss,
1990), hydrocarbon fuels (Denisov & Kovalev, 1990), lubricants
(Kuliev, 1972), edible fats and oils (Emanuel & Lyaskovskaya,
1961), cosmetics, drugs etc. Autooxidation of substrate RH proceeds
as free radical chain process with participation of
free radicals R• and RO2• and formation of hydroperoxide ROOH
(Emanuel et al., 1967; Mill & Hendry, 1980; Denisov &
Khudyakov, 1987; Denisov & Afanas’ev, 2005). The kinetic scheme
of chain oxidation of a hydrocarbon is presented below.
R
RO2RH
O2ROOH
Phenols (ArOH) act as chain breaking inhibitors of this process.
They stop developing of chain oxidation by reacting with peroxy
radicals (Emanuel et al., 1967; Mill & Hendry, 1980; Denisov
& Khudyakov, 1987; Roginsky, 1988; Denisov & Azatyan, 2000;
Denisov & Afanas’ev, 2005; Lucarini & Pedulli, 2010).
RO2• + ArOH → ROOH + ArO•
RO2• + ArO• → Molecular products
The first reaction is the limiting step of chain termination.
The rate and activation energy of this reaction depends on the
dissociation energy of O−H bond of reacting phenol and
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
406
formed hydroperoxide. So, these characteristics of phenols and
hydroperoxides are the key values in thermodynamics of
antioxidative action of phenols. Natural phenols play very
important role in preventing free radical oxidation in living
bodies. Vitamin E (tocopherols) is present in cellular membranes
and edible oils and
functions as efficient inhibitor of lipid peroxidation in
biomembranes (Burton & Ingold,
1986; Denisov & Afanas’ev, 2005). Polyfunctional phenols
(flavonoids, flavones etc.) play
important role in the biology of plants (regulation of gene
expression, gene silencing,
organization of metabolic pathways) (Grotewold, 2006). The bond
dissociation energies for
such biologically important phenols were estimated recently
(Denisov & Denisova, 2009).
2. Experimental methods of estimation of dissociation energy of
O−H bonds of phenols
2.1 Calorimetric method
The most of phenoxyl radicals are unstable and rapid disappear
by reactions of
recombination and disproportionation (Denisov & Khudyakov,
1987; Roginsky, 1988;
Denisov & Afanas’ev, 2005). However, there are a few stable
phenoxyl radicals and one of
them is 2,4,6-tri-tert-butylphenoxyl. In contrast to most free
radicals, solutions of the 2,4,6-
tri-tert-butylphenoxyl radical may be prepared and these
solutions are stable in the absence
of oxygen and other reactive compounds. This unique property was
used by L. Mahoney et
al. for to perform the direct calorimetric determination of the
heat of its reaction in systems
were the heats of formation of the other reactants and products
are known. The following
reaction was chosen for such study (Mahoney et al., 1969).
O OH ++2 2PhNH-NHPh N=N
Ph
Ph
In the result of this reaction all molecules of hydrazobenzene
are transformed into trans-
azobenzene when phenoxyl is taken into excess.
The calorimeter with base line compensator and sample injection
assembly was used for this
study. Plots of the calories absorbed vs. moles of compound
dissolved were linear with
essentially zero intercepts. The values of the partial molar
enthalpies of solution at infinite
dilution for phenol and for azobenzene were not altered by the
presence of the 2,4,6-tri-tert-
butylphenoxyl radical in the solvent. For the determination of
the heats of reaction of the
2,4,6-tri-tert-butylphenoxyl with hydrazobenzene a concentrated
solution of the radical (0.2
− 0.5 M) was used. The enthalpy of reaction was measured in
three solvents: CCl4, C6H6 and PhCl. The enthalpies of solid
reactants solution were estimated and were found to be equal
(in benzene): 13.2 kJ/mol for ArOH, 11.8 kJ/mol for analogue of
ArO•, 19.7 kJ/mol for PhNHNHPh, and 21.1 kJ/mol for trans-PhN=NPh.
They were taken into account at
calculation of enthalpy of reaction (ΔH). From the last the
difference of enthalpies was calculated:
∆Hf0(ArO•) − ∆Hf0(ArOH) = 121.9 ± 0.4 kJ/mol (298 K, 1 atm.,
benzene) (1)
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
407
As well as this difference is equal to DO−H + ∆Hf0(H•) and
∆Hf0(H•) = 218 kJ/mol (Lide, 2004) the DO−H = 339.9 kJ/mol. The
following values of reactant and product were used at this
calculation: ∆Hf0(PhNHNHPh) = 221.3 kJ/mol and
∆Hf0(trans-PhN=NPh) = 320.0 kJ/mol. Recently the following
correction was proposed with using the new value of
∆Hf0 (trans-PhN=NPh) = 310.4 kJ/mol according that DO−H = 335.1
kJ/mol (Mulder et al., 2005).
2.2 Chemical Equilibrium (CE)
The value of DO−H of 2,4,6-tri-tert-butylphenol appeared to be
very claiming in the method of
chemical equilibrium due to stability of formed phenoxyl
radical. Chemical equilibrium
Ar1O• + AriOH Ar1OH + AriO•
where Ar1O• and AriO• are reactive free phenoxyl radicals,
cannot bе achieved in solution
owing to very fast recombination or disproportionation of these
species. Such an
equilibrium can bе attained only when both radicals are stable
and do not enter the recombination reaction. In this case the
equilibrium concentrations оf both radicals can bе determined bу
electron paramagnetic resonance spectroscopy or
spectrophotometrically (Mahoney & DaRooge, 1975; Belyakov at
al., 1975, Lucarini at al., 1994). The equilibrium
constant (K) is calculated from the ratio of the equilibrium
concentrations of the molecules
and radicals:
[Ar OH] [Ar O ]1 i
[Ar OH] [Ar O ]i 1
K
•∞ ∞= •∞ ∞ (2)
The equilibrium enthalpy (ΔН) is calculated from the temperature
dependence of equilibrium constant К. On the other hand, the
equilibrium enthalpy of this reaction is equal to the difference
between the dissociation energies (DO−H) of the bonds involved in
the
reaction
ΔН = DO−H(AriOH) − DO−H (Ar1OH) (3)
provided that solvation of reactants makes an insignificant
contribution to the
equilibrium. This can bе attained bу carrying out experiments in
no polar solvents. As the reference phenoxyl radical ArlO
• were used 2,4,6-tri-tert-butylphenoxyl ((Mahoney &
DaRooge, 1975; Lucarini at al., 1994), galvinoxyl (Belyakov at al.,
1975), and ionol
(Lucarini et al., 2002). Calculations of the equilibrium
constant K from the reactant
concentration ratio were followed bу calculations of the Gibbs
free energy of equilibrium:
ΔG = −RTlnK (4)
The equilibrium enthalpy was determined using the temperature
dependence of the
equilibrium constant. Experience showed that in such reactions
one has ΔН ≅ ΔG within the limits of error in measurements. The
dissociation energies of the O−H bonds in phenols thus measured are
listed in Таblе 1.
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
408
It was found that this approach can also bе used in studies of
the systems characterized bу recombination of phenoxyl radicals
formed. Here, the reaction conditions are chosen in such
а fashion that the equilibrium between reactants is attained
rapidly and the phenols are consumed slowly, so it is possible to
monitor each reactant and calculate the equilibrium
constant. This allowed the range of phenols with known O−H bond
dissociation energies to bе extended. Having determined the
equilibrium constant, it is possible to estimate the O−H bond
strength difference between two phenols. То calculate the absolute
value of DO−H, one must know the DO−H value for one phenol. For
2,4,6-tri-tert-butylphenol, DO−H = 339.9 kJ/mol (see
2.1), which is in good agreement with the DO−H value for
unsubstituted phenol (DO−H = 369.0
kJ/mol, see (Denisov & Denisova, 2000). For galvinol, DO−H =
329.1 kJ/mol. The error in
estimating DO−H values is only 1.1 kJ/mol (Lucarini at al.,
1994). When equilibrium between
AriO and Ar1OH was studied in the solvent (S) that forms
hydrogen bond with phenol, the
difference in hydrogen bond enthalpies was taken into account.
The point of difference is
that sterically no hindered phenols form hydrogen bond Ar1OH…S
and 2,4,6-tri-tert-
butylphenol (Ar1OH) practically does not. Therefore the enthalpy
of hydrogen bond
Ar1OH…S should be abstracted from enthalpy of equilibrium. For
example, hydrogen bond
enthalpy ΔH(C6H5OH…C6H6) = −4 kJ/mol (Mulder et al., 2005). In
order to evaluate the dissociation energies of 《−H bonds in various
phenols, Mahoney and DaRooge (Mahoney & DaRooge, 1975) measured
the equilibrium constant K = k1/k−1 for
the reactions
k1
RO2 + AriOH ROOH + AriO k−1
То this end, 9,10-dihydroantracene (RH) was oxidized with oxygen
in the presence of corresponding hydroperoxide (ROOH) and phenol
(Аri《〉) at 333 K with azoisobutyronitryl as initiator. The
experimental conditions were chosen in such а manner that the
equilibrium was established in the system and the chain termination
step was
limited bу the recombination of AriO and ROO radicals. In this
case the rate (v), of the chain oxidation process is satisfactorily
described bу the following equation:
[ROOH]
1[RH]2 [ArOH]
1
−=i
k viv kp k k
t
, (5)
where kp and kt аrе the rate constants fоr the reactions of RO2
with RH and RO2 with Аr《, respectively, and vi is the initiation
rate. The dependence of the chain oxidation rate v on the
ROOH and Аr《〉 concentrations was used to determine the
kp/(2ktK)1/2 ratio and then the equilibrium constant K = k1/k−1 was
calculated using known values of ratio
kp(2kt)−1/2. The ΔD = D(ArO−H) – D(ROO−H) values were determined
assuming that ΔH = ΔG = −RTlnК. The values of D(ArO−H) calculated
relative to the O−H bond dissociation energy of sec-ROOH (365.5
kJ/mol) аrе listed in Таblе 1. The values of DO−H measured for the
same phenol in different papers are in good agreement. For example,
for 4-methylphenol
(para-cresol) DO−H = 360.7 ± 1.0 kJ/mol, for 4-tert-butylphenol
DO−H = 359.1 ± 1.6 kJ/mol, for 4-methoxyphenol DO−H = 348.2 ± 1.1
kJ/mol.
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
409
Substituents of Phenol, Phenol
Ar1OH or ROOH ΔD, kJ/mol
D, kJ/mol
Ref
3-Me ROOH −2.5 363.0 Howard & Ingold, 1965 4-Me ROOH −3.7
361.8 Howard & Ingold, 1965
4-Me ROOH −6.1 359.4 Mahoney & DaRooge, 1975
4-Me 2,4,6-tri-tert-butylphenol
20.9 360.8 Lucarini & Pedulli, 2010
4-CMe3 ROOH −4.6 360.9 Howard & Ingold, 1965
4-CMe3 ROOH −6.0 359.5 Mahoney & DaRooge, 1975
4-CMe3 2,4,6-tri-tert-butylphenol
17.1 357.0 Lucarini & Pedulli, 2010
4-Ph ROOH −12,5 353.0 Mahoney & DaRooge, 1975
2-OMe 2,4,6-tri-tert-butylphenol
19.2 359.1 Lucarini & Pedulli, 2010
3-OMe ROOH 0.7 364.8 Howard & Ingold, 1965
4-OMe ROOH −16.5 349.0 Howard & Ingold, 1965
4-OMe ROOH −16.6 348.9 Mahoney & DaRooge, 1975
4-OMe 2,4,6-tri-tert-butylphenol
6.7 346.6 Lucarini & Pedulli, 2010
3-COOEt ROOH 7.8 373.3 Mahoney & DaRooge, 1975
4-NH2 2,4,6-tri-tert-butylphenol
−12.1 327.8 Lucarini & Pedulli, 2010
4-Cl ROOH 1.9 367.4 Howard & Ingold, 1965
2-Me, 6-Me ROOH −15.3 359.2 Howard & Ingold, 1965
2-Me, 6-Me 2,4,6-tri-tert-butylphenol
13.8 353.7 Lucarini & Pedulli, 2010
3-Me, 5-Me 2,4,6-tri-tert-butylphenol
22.6 362.5 Lucarini & Pedulli, 2010
2-Me, 6-CMe3 ROOH −20.1 345.4 Howard & Ingold, 1965 2-CMe3,
6-CMe3 ROOH −11.1 354.4 Howard & Ingold, 1965
2-CMe3, 6-CMe3 ROOH −12.2 353.3 Mahoney & DaRooge, 1975
2-CMe3, 6-CMe3 2,4,6-tri-tert-butylphenol
6.7 346.6 Lucarini & Pedulli, 2010
3-CMe3, 5-CMe3 ROOH −4.5 361.0 Mahoney & DaRooge, 1975
3-CMe3, 5-CMe3 2,4,6-tri-tert-butylphenol
22.6 362.5 Lucarini & Pedulli, 2010
2-OMe, 4-Me 2,4,6-tri-tert-butylphenol
11.3 351.2 Lucarini & Pedulli, 2010
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
410
2-OMe, 4-OMe 2,4,6-tri-tret-butylphenol
4.2 344.1 Lucarini & Pedulli, 2010
3-OMe, 5-OMe 2,4,6-tri-tret-butylphenol
23.0 362.9 Lucarini & Pedulli, 2010
2-OMe, 6-OMe 2,4,6-tri-tert-butylphenol
8.4 348.3 Lucarini & Pedulli, 2010
2-Me, 4-Me, 6-Me 2,4,6-tri-tert-butylphenol
6.3 346.2 Lucarini & Pedulli, 2010
2-Me, 4-CN, 6-Me ROOH 2.5 368.0 Howard & Ingold, 1965
2-CMe3, 4-Me, 6-CMe3 Galvinol 14.6 343.7 Belyakov at al.,
1975
2-CMe3, 4-Me, 6-CMe3 2,4,6-tri-tert-butylphenol
0.3 340.2 Jackson & Hosseini, 1992
2-CMe3, 4-Me, 6-CMe3 2,4,6-tri-tert-butylphenol
−0.8 339.1 Lucarini & Pedulli, 2010
2-CMe3, 4-CMe3, 6-CMe3 Galvinol 11.5 340.6 Belyakov at al.,
1975
2-CMe3, 4-CH2Ph, 6-CMe3 Galvinol 6.9 336.0 Belyakov at al.,
1975
2-CMe3, 4-Ph, 6-CMe3 Galvinol 9.7 338.8 Belyakov at al.,
1975
2-CMe3, 4-Ph, 6-CMe3 2,4,6-tri-tert-butylphenol
0.0 339.9 Lucarini & Pedulli, 2010
2-CMe3, 4-CH=CHPh, 6-CMe3
2,4,6-tri-tert-butylphenol
−9.6 330.3 Lucarini & Pedulli, 2010
2-CMe3, 4-OMe, 6-CMe3 Galvinol −2.7 325.7 Belyakov at al.,
1975
2-CMe3, 4-OMe, 6-CMe3 2,4,6-tri-tert-butylphenol
−13.5 326.4 Jackson & Hosseini, 1992
2-CMe3, 4-OMe, 6-CMe3 2,4,6-tri-tert-butylphenol
−12.1 327.8 Lucarini & Pedulli, 2010
2-CMe3, 4-OCMe3, 6-CMe3 2,4,6-tri-tert-butylphenol
−5.9 334.0 Howard & Ingold, 1965
2-CMe3, 4-OCMe3, 6-CMe3 Galvinol 2.0 331.1 Belyakov at al.,
1975
2-CMe3, 4-CHO, 6-CMe3 2,4,6-tri-tert-butylphenol
15.2 355.1 Jackson & Hosseini, 1992
2-CMe3, 4-CHO, 6-CMe3 2,4,6-tri-tert-butylphenol
12.5 352.4 Lucarini & Pedulli, 2010
2-CMe3, 4-C(O)Me, 6-CMe3 Galvinol 24.1 353.2 Belyakov at al.,
1975
2-CMe3, 4-CH=NOH, 6-CMe3
2,4,6-tri-tert-butylphenol
−4.8 335.1 Jackson & Hosseini, 1992
2-OH, 4-CMe3, 6-CMe3, Ionol −7.1 331.5 Lucarini et al., 2002 2-
CEtMe2, 4-OH, CEtMe2, Ionol −0.8 337.8 Lucarini et al., 2002
2-CMe3, 4-CH2NMe2, 6-CMe3
2,4,6-tri-tert-butylphenol
0.7 340.6 Jackson & Hosseini, 1992
2-CMe3, 4-NO2, 6-CMe3 2,4,6-tri-tert-butylphenol
15.5 355.4 Jackson & Hosseini, 1992
2-CMe3, 4-NO2, 6-CMe3 2,4,6-tri-tert-butylphenol
15,5 355.4 Lucarini & Pedulli, 2010
2-CMe3, 4-Cl, 6-CMe3 Galvinol 16.3 345.4 Belyakov at al.,
1975
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
411
2-CMe3, 4-Cl, 6-CMe3 2,4,6-tri-tert-butylphenol
5.0 344.9 Lucarini & Pedulli, 2010
2-CMe3, 4-COOMe, 6-CMe3 2,4,6-tri-tert-butylphenol
12.1 352.0 Lucarini & Pedulli, 2010
2-CMe3, 4-COOH, 6-CMe3 2,4,6-tri-tert-butylphenol
13.0 352.9 Lucarini & Pedulli, 2010
2-CMe3, 4-CN, 6-CMe3 ROOH −7.7 357.8 Howard & Ingold,
1965
2-CMe3, 4-CN, 6-CMe3 2,4,6-tri-tert-butylphenol
12.5 352.4 Lucarini & Pedulli, 2010
2-CMe3, 4-SMe, 6-CMe3 2,4,6-tri-tert-butylphenol
−7.5 332.4 Lucarini & Pedulli, 2010
2-CMe3, 4-S(O)Me, 6-CMe3 2,4,6-tri-tert-butylphenol
6.3 346.2 Lucarini & Pedulli, 2010
2-CMe3, 4-SO2Me, 6-CMe3 2,4,6-tri-tert-butylphenol
6.7 346.6 Lucarini & Pedulli, 2010
2-CMe3, 4-CMe3, 6-SMe 2,4,6-tri-tert-butylphenol
8.8 348.7 Lucarini & Pedulli, 2010
2-OMe, 4-OMe, 6-OMe 2,4,6-tri-tert-butylphenol
−5.0 334.9 Lucarini & Pedulli, 2010
2-Me, 3-Me, 4-OMe, 6-Me 2,4,6-tri-tert-butylphenol
−8.4 331.5 Lucarini & Pedulli, 2010
2-Me, 3-Me, 4-OMe, 5-Me, 6-Me
2,4,6-tri-tert-butylphenol
2.9 342.8 Lucarini & Pedulli, 2010
2-Naphthol ROOH −6.4 359.1 Mahoney & DaRooge, 1975
Galvinol 2,4,6-tri-tert-butylphenol
−11.5 328.4 Howard & Ingold, 1965
Indol 2,4,6-tri-tert-butylphenol
−14.8 325.1 Howard & Ingold, 1965
Table 1. The values of DO−H of substituted phenols estimated by
CE method (DO−H = 339.9 kJ/mol for 2,4,6-tri-tert- butylphenol DO−H
= 329.1 kJ/mol for galvinol, and DO−H = 365.5 kJ/mol for sec-ROOH
(Denisov & Denisova, 2000))
2.3 Low pressure pyrolysis of substituted anisoles (VLPP)
The direct approach to estimation of dissociation energy of O-H
bond of phenol via reaction
C6H5OH → C6H5O• + H• cannot be successful due to the presence of
a competing tautomerization of phenol to the cyclohexa-2,4-dienon
(Zhu & Borzzelli, 2003.). An indirect way to assess the
phenolic O−H bond dissociation energy is by studying the
temperature dependence of the rate constant for O−C bond
dissociation in phenyl ethers, such as anisoles (Suryan et al.,
1989a; Suryan et al., 1989b) and benzylphenyl ether (Pratt at al.,
2001). In these studies, dissociation rates of substituted anisoles
were determined in the gas phase by a method of very-low-pressure
pyrolysis (VLPP). This method provides a straightforward means for
determining decomposition rates in the absence of bimolecular
reactions. Anisoles are especially suited
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
412
for study by this method, since their low O−Me bond strengths
(ca. 268 kJ/mol) cause them to homolyze under relatively mild (for
VLPP) conditions (800-1200 K). The decomposition of substituted
anisoles was found to proceed exclusively by simple homolysis
(Suryan et al., 1989a). General operating principles of the VLPP
technique have been described by Golden et al
(Golden et al., 1973). Anisole decomposition were performed at T
= 800 ÷ 1200 K and pressure p = 10−2 ÷ 10−4 Torr monitored
periodically and percentage dissociation was reproducible to ±1%
(Suryan et al., 1989b). An electron impact quadruple mass
spectrometer, tuned to 70-eV ionization energy, was used to monitor
reactant decomposition. Unimolecular reaction rate constants, kuni,
under VLPP conditions were calculated from the equation (Suryan et
al., 1989a).
kuni/ke = x/(1 − x) =(I0 − I)/I. (6)
where, ke, the escape rate constant is 3.965(T/M)1/2 s−1 for the
3-mm aperture reactor, M is the molecular weight, T is the
temperature (K), and x represents the fraction of reactant
decomposed. The latter value was derived from mass spectrometer
signal intensity of the parent molecular ion before reaction (I0)
and after reaction (I) at an ionization energy of 70 eV (Suryan et
al., 1989a).
2-Y 3-Y 4-Y Y
ΔD, kJ/mol
DO−H, kJ/mol
ΔD, kJ/mol
DO−H, kJ/mol
ΔD, kJ/mol
DO−H, kJ/mol
Ref
Me −10.9 358.1 −2.1 366.9 −7.9 361.1 Suryan et al., 1989b CH=CH2
−10.5 358.5 Suryan et al., 1989b OMe −17.6 351.4 −4.6 264.4 −16.3
352,7 Suryan et al., 1989a OMe −17.1 351.9 −13.0 356.0 Pratt at
al., 2001 C(O)Me −6.0 333.9 0.8 369.8 2.5 371.5 Suryan et al.,
1989b OH −29.9 310.0 1.2 370.2 −10.5 358.5 Suryan et al., 1989a OH
−30.1 338.9 −11.3 357.7 Pratt at al., 2001 NH2 −30.9 309.8 −1.7
367.3 −12.5 356.5 Suryan et al., 1989b CN −0.9 339.0 −0.4 368.6 1.2
370.2 Suryan et al., 1989b NO2 −5.6 334.3 −2.1 366.9 4.6 373.6
Suryan et al., 1989b F −8.0 361.0 3.8 372.8 −4.6 264.4 Suryan et
al., 1989b Cl −9.2 359.8 0.8 369.8 −4.6 264.4 Suryan et al., 1989a
Br −7.1 361.9 Suryan et al., 1989a CF3 9.2 378.2 Pratt at al.,
2001
Table 2. Dissociation energies of O−H bonds (in kJ/mol) in
substituted phenols estimated by VLPP technique, DO−H(C6H5OH) =
369.0 kJ/mol
For a meaningful comparison of rate constants for the different
reactions, they were converted to their high-pressure
(collision-frequency independent) values. This was done
with RRKM theory (Robinson & Holbrook, 1972). The
pre-exponential A factor of 1015.5 s−1 was assumed for all
reactions. Activation energies were used for to calculate DO−C at
standard conditions using the equation (Mulder et al., 2005):
DO−C = Euni + RTm − ΔCp(Tm −298), (7)
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
413
where Tm is the average temperature of experiment, ΔCp is the
average change in heat capacity between Tm and T = 298 K. The
errors in rate constants, measured at 50%
decomposition, were approximately 10%.
As well as the enthalpy of exchange reaction
PhOH + YC6H4OMe YC6H4OH + PhOMe
was proved to be very small (Suryan et al., 1989a) one can use
the differences in dissociation
energy of C−O bonds of substituted anisoles for evaluation of
dissociation energy of O−H bonds of phenols. The results of
calculation of dissociation energy for O−H bonds in substituted
phenols taking into account DO−H(C6H5OH) = 369.0 kJ/mol (Denisov
&
Denisova, 2000) are presented in Table 2.
2.4 Estimation of bond dissociation energy from kinetic
measurements
In the framework of the intersecting parabolas model (MIP) the
transition state of а radical reaction, for example
RO2• + ArOH → ROOH + ArO•
is treated as а result of intersection of two potential energy
curves (Denisov, 1997; Denisov, 1999; Denisov & Denisova, 2000;
Denisov & Afanas’ev, 2005; Denisov et al., 2003). One of
them characterises the potential energy of the stretching
vibration of the attacked ArO−H bond as а function of the vibration
amplitude while the other characterises the potential energy of the
vibration of the ROO−H bond being formed. The stretching vibrations
of the bonds are considered harmonic. A free radical abstraction
reaction is characterised bу the following parameters:
1. classical enthalpy ΔHe. which includes the zero-point
vibrational energy difference between the bond being cleaved and
the bond being formed;
2. classical potential activation barrier Ее which includes the
zero-point vibrational energy of the bond being cleaved;
3. parameter rе equal to the total elongation of the bond being
cleaved and the bond being
formed in the transition state;
4. coefficient b (2b2 is the force constant of the bond being
cleaved);
5. parameter α (α2 is the force constant ratio of the reacting
bonds); 6. pre-exponential factor А0 per equally reactive cleaved
bond (in the molecule) involved
in the reaction. The rate constant is expressed via Arrhenius
equation: k =
nOHA0exp(−E/RT) where nOH is a number of OH groups with
equireactivity. All these values are connected via equation:
e e e eα= + Δ +br E H E . (8) The MIP method allows the variety
of radical reactions to bе divided into classes using experimeпtal
data. Each class is characterised bу the same set of parameters
mentioned above. An individual reaction belonging to а certain
class is characterised bу the classical enthalpy He and classical
activation energy Ее that for the written above reaction is
expressed by the equation (at ΔHe(1 − α2)
-
Application of Thermodynamics to Biological and Materials
Science
414
Ee = 0.496 bre + 0.507 (bre)−1ΔHe, (9) were parameter bre =
13.16 (kJ/mol)1/2 for reaction RO2
• + phenol and bre = 14.30 (kJ/mol)1/2 for reaction RO2
• + sterically hindered phenol (Denisov & Denisova, 2000). А
method for estimating the bond strengths from the kinetic data
developed in the framework of the MIP model, involves а number of
versions (Denisov, 1995a; Denisov, 1995b; Denisov, 1997; Denisov,
1999; Denisov & Tumanov, 2005). 1. With the measured rate
constants ki or the ki/kl ratios for а reaction class of the
type
RO2• + ArOH it is possib1e to estimate the difference in bond
strengths between the
AriOH and Ar1OH compounds. Тhе rate constant ratio ki/kl allows
to calculate the activation energies difference:
ΔEi = Ei – E1 = RTln(nik1/n1ki) (10) where n1 and ni are
respectively the numbers of equally reactive bonds in the Ar1OH
and AriOH molecules attacked bу the RO2• radical. From Eqn. (8)
it follows that the relation between the ΔEi value and the enthalpy
difference Δ(ΔHi) between these reactions has the form:
Δ(ΔHi) = 1.945 bre ( 1 1+ Δ −E E Ee ei ) + 0.0274 ΔEi (11) 《n
the other hand, the enthalpy difference Δ(ΔHi) = Di − D1 and the
strength of the AriO−H bond сan bе calculated using the
equation:
Di = D1 + 1.945 bre ( 1 1+ Δ −E E E
e ei) + 0.0274 ΔEi (12)
Thus, calculations of the Di values require knowledge of the D1,
Ee1, k1/ki ratio, and the
parameters characterising а given reaction class (parameter bre
and coefficient α). Experience showed that the error in ΔD
measurements is 1.5 ÷ 2.5 kJ/mоl.
2. Using different radicals (e.g. RiOO•) in а series of radical
reactions RiOO• + RH
belonging to the same class allows the approach to bе employed
for evaluating the RiOO−H bond strengths. In this case Eqn. (12)
takes the form:
Di = D1 + 2α−2bre ( 1 1− + ΔE E Ee e i ) + (α−2−1)ΔEi (13) where
Ee1 refers to reaction R1O2
• + RH, coefficients α and bre see in Handbook (Denisov &
Denisova, 2000). This version of the technique was used in
estimating the DO−H
values in hydroperoxides (see 4.1).
3. The Di value for а free radical abstraction reaction саn also
bе evaluated from the absolute value of the rate constant ki.
(Denisov & Tumanov, 2005). Limitation imposed on the method is
associated with the enthalpy of reaction (Denisov,
1997; Denisov & Denisova, 2000). The case in point is that
Eqn (8) is valid for reactions
belonging to the same reaction class and characterised bу
enthalpies lying in the interval ΔHemin < ΔНе < ΔНеmах. Тhе
activation energy for а highly exothermic reaction (ΔНе <
ΔHemin) is nearly zero (more correctly, Е = 0.5RT) and independent
of ΔН. Therefore the enthalpies ΔНе of these reactions cannot bе
estimated from the Ее values. Тhе ΔHemin vа1uе depends on the bre
and α parameters and on the zero-point
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
415
vibrational energy of the bond being cleaved. Тhе activation
energies of highly endothermic reactions (Не > ΔНеmах) is
approximately equal to ΔН:
Е = ΔН + 0.5 RT. (14) The bond dissociation energies estimated
from experimental data on reactions of peroxyl radicals with
phenols in hydrocarbon solutions are given in Table 3.
Phenol, YC6H4OH 2,6-Di-tert-butylphenol Substituents of Phenol,
Phenol ΔDO−H, kJ/mо1 DO−H, kJ/mо1 ΔDO−H, kJ/mо1 DO−H, kJ/mо1 H 0.0
369 7.7 347.6
2-Me −9.1 359.9 3-Me −2.3 366.7 4-Me −6.8 362.2 0.0 339.9 2-CMe3
−15.2 353.8 4-CMe3 −8.9 360.1 0.0 339.9 4-Ph −1.3 338.6 4-CH2Ph 0.7
340.6
4-CMe2Ph 1.1 341.0
4-CHPh2 3.3 343.2
4-OMe −8.3 331.6 4-OCMe3 −21.2 347.8 −7.9 332.0 2-OH −29.4 339.6
3-OH 0.1 369.1
4-OH −17.0 352.0 4-COOH 2.7 371.7 9.8 349.7
4-C(O)H 8.8 348.7
4-C(O)Me 6.5 346.4
4-COOCMe3 8.8 348.7
4-CH2COOH −2.3 337.6 4-CH2COOMe 3.8 343.7
4-(CH2)2COOC18H37 0.6 340.5
4-CH2NH2 −4.2 335.7 4-NHAc −12.3 327.6 4-NO 7.0 346.9
4-NO2 3.8 372.8 19.0 358.9
4-CN 13.4 353.3
4-Cl 5.5 345.4
4-SPh 7.4 347.3
2-Me, 3-Me −13.5 355.5 2-Me, 4-Me −8.5 360.5
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
416
2-Me, 6-Me −14.4 354.6 3-Me, 4-Me −14.4 354.6 3-Me, 5-Me −4.3
364.7 2-Me, 4-CMe3 −9.1 359.9 2-CMe3, 4-CMe3 −9.5 359.5 3-CMe3,
5-CMe3 −6.6 362.4 2-CMe3, 4-OMe −25.6 343.4 2-OH, 4-CMe3 −26.6
342.4 2-Me, 4-OH −19.2 349.8 2-Me, 4-Me, 6-Me −21.5 347.5 2-Me,
4-Me, 5-Me −12.2 356.8 2-CMe3, 4-Me, 6-Me −13.2 355.8 2-CMe3,
4-CMe3, 6-CMe3 −13.1 355.9 2-Me, 4-CH2NH2, 5-Me −20.9 348.1 2-Me,
4-Cl, 5-Me −17.6 351.4 2-S(CH2)2CN, 4-Me, 6-CHMePh −21.5 347.5
2-Me, 4-CH2NH2, 6-CMe3 −18.4 350.6 2-Me, 3-Me, 4-Me, 6-Me −21.4
347.6 2-Me, 3-Me, 5-Me, 6-Me −17.8 351.2 2-Me, 3-Me, 4-Me, 5-Me,
6-Me −28.5 340.5 2-OH, 3-CMe3, 5-CMe3 −28.7 340.3 2-OH, 3-CMe3,
6-CMe3 −29.5 339.5 3-Me, 4-CH2COOH, 5-Me −19.0 350.0 2-Me, 4-CH2CN,
6-Me −15.0 354.0 2-Me, 3-Me, 4-OH, 5-Me −24.3 344.7 2-OMe, 3-OMe,
4-OH, 6-Me −25.2 343.8 1-Naphthol −25.6 343.4 2-Naphthol −15.2
353.8 1-Hydroxyfluorene −30.7 338.3 1-Hydroxyphenanthrene −14.3
354.7 2-Hydroxyphenanthrene −2.0 367.0 3-Hydroxyphenanthrene −6.5
362.5 4-Hydroxyphenanthrene −12.8 356.2 3,8-Pyrendiol −53.1 315.9
3,10-Pyrendiol −51.3 317.7
Table 3. The values of DO−H for phenols estimated by MIP
(Denisov, 1995a; Denisov & Denisova, 2000)
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
417
2.5 Photoacoustic calorimetry (PAC)
Photoacoustic calorimetry is a thermodynamic method of
estimation of bond dissociation
energies in solution. The physical principle of PAC is the
following (Rothberg et al., 1983;
Simon & Peters, 1983; Grabowski et al., 1984). Very rapid
heat release from a photoinitiated
process in liquid generates a pressure wave. This wave
propagates through the solution at
the speed of sound. Detection and quantification of this
pressure wave is the bases of the
technique.
The values of dissociation energies of O−H bonds in phenols were
estimated by (Wayner et al., 1995; Wayner et al., 1996; Laarhoven
et al., 1999). Di-tert-butyl peroxide was used as
photoinitiator. Pulses from a nitrogen laser (λ = 337.1 nm;
pulse width 10 ns; power, 10 mJ per pulse; repetition rate, 5 Hz)
were used to photolyse di-tert-butyl peroxide in solution.
Me3COOCMe3 + hν → 2 Me3CO The formed tert-butoxy radicals react
very rapidly with phenol with evolution of heat.
Me3CO + ArOH → Me3COH + ArO
Substituents of Phenol ΔD, kJ/mol D, kJ/mol
4-H 0.0 369.0
4-CMe3 −7.9 361.1 4-OMe −24.3 344.7 4-CF3 13.4 382.4
4-CN 23.4 392.4
4-Cl 1.7 370.7
2-Me, 4-Me, 6-Me- −23.0 346.0 2-CMe3, 4-Me, 6-CMe3 −32.2 336.8
2-CMe3, 4-CMe3 −21.8 347.2 2-Me, 4-OMe, 6-Me- −42.3 326.7
Table 4. Dissociation energies of O−H bonds of phenols measured
by PAC, benzene, T = 298 K, (Wayner et al., 1996; Laarhoven et al.,
1999)
An iris ensured that only a very small part of the light passed
as a fine beam through the centre of the cell, and a low powered
lens was used to correct for the slight divergence of the beam. The
heat evolved as a result of the photoinitiated reactions caused a
shock wave in the solution, which was transmitted at the speed of
sound to the cell wall. Here, the primary wave and its many
reflections were detected in a time-resolved mode by a
piezoelectric transducer. The transducer signals were amplified and
were recorded on a storage oscilloscope. A quartz plate was used to
reflect part of the laser beam to a reference device, so that
corrections could be made for variations in the laser power. On
prolonged irradiation some drift in this device occurred,
presumably because small convection currents were set up in the
solution. However, the problem was easily
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
418
overcome by slowly flowing the solution through the cell with a
peristaltic pump. Signals from the reference transducer were
amplified and were stored in a second channel of the oscilloscope.
The time profiles of the photoacoustic waves were quite
reproducible so long as the geometry of the apparatus remained
unchanged. The measurements from a line of laser shots were
averaged to give the amplitudes of the photoacoustic waves due to
sample and reference. In the photoacoustic experiment, an important
condition was that the heat evolved in a given reaction was
released in a time that was short with respect to the response of
the transducer. This was tested by different ways. The samples used
in the photoacoustic experiments were always carefully deoxygenated
by nitrogen or argon purging and were flowed through the cuvette so
as to avoid problems associated with sample depletion and product
formation. Samples that were oxygen-sensitive were always prepared
in an inert atmosphere since oxidation generally gave rise to
colored impurities which affected the optical properties of the
solutions. The results of DO−H estimation of a line substituted
phenols are listed in Table 4. The results on DO−H estimation in
C6H5OH see in paragraph 3.
2.6 Acidity − oxidation potential method (AOP) The theoretical
basis for acidity − oxidation − potential method (AOP) (Bordwell
& Bausch, 1986; Bordwell et al., 1991) lies in thermochemical
cycle:
ArOH ArO− + H+ (pKa)
ArO− ArO• + e− (Eox(ArO−))
H+ + e− H• (Er(H+))
ArOH ArO• + H• (DO−H) Equilibrium acidity measurements and
oxidation potentials, both measured in Me2SO solution and can be
combined to obtain relative homolytic dissociation energy of O−H
bond of phenol. Since Ered for the proton is constant, differences
in the sum of the oxidation potentials of the anions and the
acidity constants for their conjugate acids (pK) can be taken as
measures of relative bond dissociation energy:
ΔDO−H(kJ/mol) = 5.73ΔpKArOH + 96.48ΔEox(ArO−) (15) This approach
is limited in practice by the irreversibility of the oxidation
potentials for most anions. Nevertheless, there was observed that
when families of anions wherein basicities have been changed by
remote substitution are used, good correlations between Eox and
pKArOH, or between Eox and log k for electron-transfer reactions,
are often obtained. In these instances, the extent of
irreversibility of Eox throughout the family appears to be similar
enough to permit estimates of relative bond dissociation energies
by this method. Lind et al. measured the constant of equilibrium in
aqueous solution:
ArO− + ClO2• ArO• + ClO2−
using pulse radiolysis technique (Lind et al., 1990). The values
of ΔDO−H estimated by two methods are listed in Table 5.
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
419
Substituents of Phenol, Phenol
ΔDO−H, kJ/mol, (Bordwell & Cheng, 1991)
ΔDO−H, kJ/mol, (Arnett et al., 1990)
ΔDO−H, kJ/mol, (Lind et al., 1990)
H 0.0 0.0 0.0 2-Me −6.9 3-Me −1.9 4-Me −4.8 −18.7 −0.9 3-Me,
5-Me −3.1 2-Me, 6-Me −18.2 4-CMe3 −4.8 −7.3 2-CMe3, 6-CMe3 −32.4
2-CMe3, 4-CMe3, 6-CMe3 −32.0 4-Ph −9.4 2-OMe −16.1 3-OMe 1.5 4-OMe
−22.0 −22.2 −23.4 4-O− −70.5 −66.1 4-OH −34.9 −33.5 3-NH2 −7.7
3-NMe2 −8.2 4-NH2 −52.5 −53.1 4-NMe2 −40.0 −58.6 4-F −1.9 −3.3 2-Cl
0.6 3-Cl 8.2 4-Cl 1.9 7.5 −2.5 3-Cl, 5-Cl 16.9 3-Cl, 4-Cl , 5-Cl
13.6 4-Br 3.6 −0.4 4-I −1.2 3-CF3 16.5 4-CF3 22.8 3-SO2Me 10.2
4-SO2Me 21.5 3-C(O)Me 8.2 4-C(O)Me 12.3 2.1 4-C(O)Ph 11.1 4-OC(O)Me
−11.5 4-CO2− 7.1 3-CN 16.9 4-CN 18.2 6.1 19.7 3-NO2 18.6 4-NO2 20.3
9.1 25.1 1-Naphthol −24.5 2-Naphthol −7.7
Table 5. The values of ΔDO−H of substituted phenols measured by
electrochemical techniques
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
420
3. Dissociation energies of O−H bonds of phenols 3.1
Dissociation energy of O−H bond of C6H5OH As was shown earlier, the
O−H bond of simplest phenol C6H5OH plays a key role among a line of
different substituted phenols. The absolute value of DO−H(ArOH) can
be calculated via difference of bond dissociation energies: ΔDO−H =
DO−H(ArOH) − DO−H(C6H5OH) and the last can be estimated by a line
of methods. The values of DO−H(C6H5OH) were measured during last 20
years and are collected in Table 6. Year DO−H(C6H5OH), kJ/mol
Method Ref. 1989 374.5 VLPP (gas) Suryan et al., 1989a 1990 369.5
Shock tube (gas) Walker & Tsang, 1990 1991 375.9 AOP (Me2SO)
Bordwell & Cheng, 1991 1995 365.3 PAC (C6H6) Wayner et al.,
1995 1996 369.4 CE (C6H6) Lucarini et al.,1996 1998 376.6 Negative
ion cycle (gas) DeTuri & Ervin, 1998 2000 369.0 Recommended
Denisov & Denisova, 2000 2003 368.2 Recommended Luo, 2003 2004
359.0 Negative ion cycle (gas) Angel & Ervin, 2005 2005 362.3
Recommended Mulder et al., 2005
Table 6. The values of DO−H(C6H5OH) estimated by different
techniques
It is seen from Table 6 that experimental values of DO−H(C6H5OH)
vary from 359 to 377
kJ/mol, the mean value of DO−H(C6H5OH) = 369.0 ± 5.7 kJ/mol.
This value coincides with that recommended in Handbook (Denisov
& Denisova, 2000) and the last is in good agreement with DO−H
of hydroperoxides (see paragraph 4). In recent years, quantum
chemical methods, particularly density functional theory, are often
used for the assessment of the dissociation energy of O−H bond in
phenols. Let us know that the results of calculation as a rule,
differ substantially from the experimental values. As
we see experimental DO−H(C6H5OH) = 369 ± 6 kJ/mol and calculated
values are sufficiently lower (see Table 7).
Method DO−H, kJ/mol
Method DO−H, kJ/mol
6-31G 332.8 6-31+G(d,p) 344.2 6-31G(d) 327.7 6-311+G(d,p) 347.5
6-31G(d,p) 346.2 6-311+G(2d,p) 348.0 6-31G(d,p) 341.7
6-311+G(2d,2p) 350.7 6-31G(d,p’) 361.3 6-311+G(3d,p) 350.1
6-31+G(d) 328.9 G-3 369.0
Table 7. Values of DO−H(C6H5OH) calculated by density functional
theory (Wright et al., 1997; Luzhkov, 2005; Mulder et al.,
2005)
3.2 Dissociation energies of O−H bond of substituted phenols As
was shown earlier, the influence of substituent of aromatic ring on
DO−H is very important. As well as each technique has its specific
peculiarities that may influence on the measured
value ΔDO−H it would be useful to compare them. This comparison
is performed in Table 8.
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
421
CE VLPP MIP AOP PAC Substituents of Phenol, Phenol ΔD,
kJ/mol ΔD, kJ/mol
ΔD, kJ/mol
ΔD, kJ/mol
ΔD, kJ/mol
D, kJ/mol
2-Me −10.9 −9.1 −6.9 360.0 ± 1.6 3-Me −6.0 −2.1 −2.3 −1.9 365.9
± 1.7 4-Me −8.3 ± 1.0 −7.9 −6.8 −4.8 361.6 ± 1.3 4-CMe3 −10.0 ± 1.6
−8.9 −4.8 −7.9 361.1 ± 0.5 4-Ph −16.0 −9.4 356.3 ± 3.3 3-OH 1.2 0.1
368.4 ± 0.7 4-OH −10.9 ± 0.4 −17.0 −34.9 (?) 355.1 ± 3.0 2-OMe −9.9
−17.6 −16.1 354.5 ± 3.3 3-OMe −4.2 −4.6 1.5 (?) 364.6 ± 0.2 4-OMe
−20.8 ± 1.1 −14.6 ± 1.7 −22.0 −24.3 346.6 ± 1.4 3-NH2 −1.7 −7.7
364.3 ± 3.0 4-NH2 −41.2 −12.5 (?) −52.5 322.2 ± 5.6 3-CN −9.4 16.9
(?) 359.6 4-CN 1.2 18.2 23.4 389.8 ± 2.6 3-NO2 −2.1 18.6 (?) 366.9
4-NO2 4.6 3.8 20.3 373.2
4-F −4.6 −2.6 365.4 2-Cl −9.2 0.6 (?) 359.8 3-Cl 0.8 8.2 (?)
369.8
4-Cl −1.6 −4.6 1.9 1.7 368.4 ± 2.7 4-CF3 9.2 22.8 (?) 378.2
2-Me, 6-Me −12.5 ± 2.7 −18.2 353.7 ± 2.8 3-Me, 5-Me −6.5 −3.1
364.2 ± 1.7 3-CMe3, 5-CMe3 −8.0 −6.6 361.7 ± 0.7 2-CMe3, 6-CMe3
−19.0 ± 3.4 −22.6 −32.4 (?) 349.1 ± 1.6 2-CMe3, 4-Me, 6-CMe3
−27.0 ± 1.5 −13.1(?) −32.0 −32.2 338.6 ± 2.4 1-Naphthol −25.6
−24.5 344.0 ± 0.6 2-Naphthol −9.9 −15.2 −7.7 358.1 ± 3.1 Indol
−43.9 −41.8 326.2 ± 1.0 Table 8. Comparison of ΔD (kJ/mol) =
D(AriOH) − D(C6H5OH) for substituted phenols estimated by various
methods, D(C6H5OH) = 369.0 kJ/mol (see Tables 1−5); data marked by
(?) were not included in the calculation of mean values of ΔD
We observe a good agreement between ΔD measured by different
methods for phenols with alkyl, alkoxyl, and amino substituents.
However, for phenols with polar electronegative substituents such
as Cl, CF3, CN, and NO2 method AOP gives much higher absolute
values of ΔD in comparison with another methods. The possible
explanation of these discrepancies lies in strong additional
solvation of polar groups in such strong polar solvent as
dimethylsulfoxide used in AOP method.
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
422
3.3 Dissociation energies of O−H bonds of natural phenols
Bioantioxidants play very important role in biological processes
and are under intensive investigation during last a few decades.
Among them only for tocopherols and ubiquinols were measured their
O−H bonds dissociation energies (Denisov & Denisova, 2000; Luo,
2003). These important characteristics for many natural phenolic
compounds (flavonoids et al.) were estimated only recently (Denisov
& Denisova, 2008). The list of these data is given in Table
9.
Phenol Site of《−〉 bond
DO−H, kJ/mol
Method Ref.
α-Tocopherol 6 328.9 CE Jackson & Hosseini, 1992
α-Tocopherol 6 330.1 CE Lucarini et al., 1996
α-Tocopherol 6 330.0 MIP Denisov, 1995
α-Tocopherol 6 327.3 CE Lucarini et al., 1994
α-Tocopherol 6 323.4 ± 8.0 PAC Wayner et al., 1996 α-Tocopherol
6 338.5 AOP Bordwell & Liu, 1996
β-Tocopherol 6 335.2 MIP Denisov & Denisova, 2009
β-Tocopherol 6 335.6 MIP Denisov, 1995 β-Tocopherol 6 335.3 ±
2.0 MIP Denisova & Denisov,
2008
γ- Tocopherol 6 334.8 MIP Denisov & Denisova, 2009
γ-Tocopherol 6 335.1 MIP Denisov 1995 γ-Tocopherol 6 334.9 ± 2.0
MIP Denisova & Denisov,
2008
δ- Tocopherol 6 341.4 MIP Denisov & Denisova, 2009
δ- Tocopherol 6 342.8 MIP Denisov, 1995 δ- Tocopherol 6 335.6
PAC Wayner et al., 1996 δ- Tocopherol 6 341.5 ± 2.0 MIP Denisova
& Denisov,
2008
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
423
Ubiquinol-0 1,4 343.8 MIP Denisov, 1995
Ubiquinol-0 1,4 346.0 MIP Denisova & Denisov, 2008
Ubiquinol-2 1,4 344.3 MIP Denisov, 1995
Ubiquinol-2 1,4 345.7 MIP Denisova & Denisov, 2008
Ubiquinol-6 1,4 344.3 MIP Denisov, 1995
Ubiquinol-6 1,4 345.7 MIP Denisova & Denisov, 2008
Ubiquinol-9 1,4 344.8 MIP Denisova & Denisov, 2008
Ubiquinol-10 1,4 345.6 MIP Denisova & Denisov, 2008
5-Hydroxy-2,4,6,7-tetramethyl-2,3-dihydrobenzo[b]furan
5 326.7 MIP Denisov & Denisova, 2009
5-Hydroxy-2,2,4,6,7-pentamethyl-2,3-dihydrobenzo[b]furan
5 326.4 MIP Denisov & Denisova, 2009
5-Hydroxy-2,2,4,6,7-pentamethyl-2,3-dihydrobenzo[b]furan
5 323.4 CE Jackson & Hosseini, 1992
5-Hydroxy-2-carboxy-2,4,6,7-tetra-methyl-2,3-dihydrobenzo[b]furan
6 334.0 MIP Denisov & Denisova, 2009
6-Hydroxy-5,7,8-trimethylchromane 6 330.9 MIP Denisov &
Denisova, 2009
6-Hydroxy-2-hydroxymethyl-2,5,7,8-tetramethylchromane
6 330.9 MIP Denisov & Denisova, 2009
6-Hydroxy-2-methoxy-2,5,7,8-tetramethylchromane
6 334.4 MIP Denisov & Denisova, 2009
6-Hydroxy-2-carboxy-2,5,7,8-tetramethylchromane
6 336.5 MIP Denisov & Denisova, 2009
6-Hydroxy-2-methylcarboxy-2,5,7,8-tetramethylchromane
6 333.3 MIP Denisov & Denisova, 2009
6-Hydroxy-2-carboxymethyl-2,5,7,8-tetramethylchromane
6 333.0 MIP Denisov & Denisova, 2009
6-Hydroxy-2-methylcarboxymethyl-2,5,7,8-tetramethylchromane
6 330.9 MIP Denisov & Denisova, 2009
6-Hydroxy-2,2,5,7,8-pentamethylchromane 6 328.9 MIP Denisov
& Denisova, 2009
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
424
6-Hydroxy-2,2,5,7,8-pentamethylchromane 6 328.4 MIP Denisova
& Denisov, 2008
6-Hydroxy-2,2,8-trimethyl-5,7-diethylchromane
6 331.9 MIP Denisova & Denisov, 2008
6-Hydroxy-2,2-dimethyl-5,7-diethylchromane
6 333.6 MIP Denisova & Denisov, 2008
6-Hydroxy-2,2,8-trimethyl-5,7-diisopropylchromane
6 337.0 MIP Denisova & Denisov, 2008
6-Hydroxy-2,2-dimethyl-5,7-diisopropylchromane
6 335.7 MIP Denisova & Denisov, 2008
6-Hydroxy-5-methyl-7-tert-butylchromane 6 332.5 MIP Denisova
& Denisov, 2008
6-Hydroxy-5-isopropyl-7-tert-butylchromane
6 340.7 MIP Denisova & Denisov, 2008
6-Hydroxytocol 6 340.1 MIP Denisova & Denisov, 2008
6-Hydroxy-5,7-diethyltocol 6 333.9 MIP Denisova & Denisov,
2008
6-Hydroxy-5,7-diethyl-8-methyltocol 6 331.9 MIP Denisova &
Denisov, 2008
6-Hydroxy-5,7-diisopropyltocol 6 335.7 MIP Denisova &
Denisov, 2008
6-Hydroxy-5,7-diisopropyl-8-methyltocol 6 336.3 MIP Denisova
& Denisov, 2008
6-Hydroxy-5-methyl-7-tert-butyltocol 6 333.2 MIP Denisova &
Denisov, 2008
6-Hydroxy-5-isopropyl-7-tert-butyltocol 6 339.3 MIP Denisova
& Denisov, 2008
6-Hydroxy-5,7,8-trimethyl-3,4-dihydro- 2H-1-benzothiopyran
6 332.5 MIP Denisova & Denisov, 2008
6-Hydroxy-2,5,7,8-tetramethyl-3,4-dihydro-2H-1-benzothiopyran
6 333.9 MIP Denisova & Denisov, 2008
6-Hydroxy-2,2,5,7,8-pentamethyl-3,4-dihydro-2H-1-benzothiopyran
6 333.4 MIP Denisova & Denisov, 2008
6-Hydroxy-2-phytyl-2,5,7,8-tetramethyl-3,4-dihydro-2H-1-benzothiopyran
6 333.3 MIP Denisov, 1995
6-Hydroxy-2-phytyl-2,5,7,8-tetramethyl-3,4-dihydro-2H-1-benzothiopyran
6 334.7 MIP Denisova & Denisov, 2008
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
425
6-Hydroxy-2-methylcarboxy-2,5,7,8-tetramethyl-
3,4-dihydro-2H-1-benzothiopyran
6 337.8 MIP Denisova & Denisov, 2008
6-Hydroxy-2,5-dimethyl-2-phytyl-7,8-benzochromane
6 321.4 MIP Denisova & Denisov, 2008
6-Hydroxy-2,5-dimethyl-2-phytyl-7,8-benzochromene
6 322.1 MIP Denisova & Denisov, 2008
6-Hydroxy-4,4,5,7,8-pentamethyl-3,4-dihydro-2H-
1-benzothiopyran
6 329.8 MIP Denisova & Denisov, 2008
5,7,8-Trimethylselenotocol 6 335.7 MIP Denisova & Denisov,
2008
5-Hydroxy-2,4-dimethyl-2,3-dihydro-benzo[b]selenophene
5 334.5 MIP Denisova & Denisov, 2008
5-Hydroxy-2-methyl-2,3-dihydro-benzo[b]selenophene
5 342.3 MIP Denisova & Denisov, 2008
Kaempferol 7,4′ 348.9 MIP Denisova & Denisov, 2008
Morin 7,4′ 363.6 MIP Denisova & Denisov, 2008
Ubichromenol 1,4 350.2 MIP Denisova & Denisov, 2008
Quercetin 4′ 343.0 MIP Denisova & Denisov, 2008
(−)-Epicatechin 4′ 346.2 ± 1.8 MIP Denisova & Denisov,
2008
(−)-Epicatechin 4′ 339.7 CE Lucarini et al., 2002
6,7-Dihydroxyflavone 6 332.3 MIP
Denisova & Denisov, 2008
7,8-Dihydroxyflavone 8 333.0 MIP Denisova & Denisov,
2008
Chrysin 7 357.1 MIP Denisova & Denisov, 2008
Galangin 7 363.1 MIP Denisova & Denisov, 2008
Dihydroquercetin 4′ 343.6 MIP Denisova & Denisov, 2008
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
426
Catechin 4′ 348.1 ± 1.3 MIP Denisova & Denisov, 2008
Hesperitin 3′ 353.8 MIP Denisova & Denisov, 2008
Fisetin 4′ 348.0 ± 1.7 MIP Denisova & Denisov, 2008
Gallic acid 4 347.4 MIP Denisova & Denisov, 2008
Propyl gallate 4 334.6 MIP Denisova & Denisov, 2008
Propyl gallate 4 339.7 CE Lucarini et al., 2002
Myricetin 4′ 340.9 MIP Denisova & Denisov, 2008
(−)-Epigallocatechin 4′ 344.6 MIP Denisova & Denisov,
2008
Rutin 4′ 343.2 ± 0.6 MIP Denisova & Denisov, 2008
Hesperidin 3′ 345.8 MIP Denisova & Denisov, 2008
Luteolin 4′ 342.7 MIP Denisova & Denisov, 2008
Nordihydroguaiaretic acid 4,4′ 351.3 MIP Denisova & Denisov,
2008
Caffeic acid 4 339.8 MIP Denisova & Denisov, 2008
(−)-Epigallocatechin gallate 4′,4′′ 338.7 ± 0.3 MIP Denisova
& Denisov, 2008
β-Glucogallin 4 335.0 MIP Denisova & Denisov, 2008
(−)-Epicatechin gallate 4′,4′′ 339.6 ± 1.3 MIP Denisova &
Denisov, 2008
Tannic acid 4 341.6 MIP Denisova & Denisov, 2008
Pentagalloylglucose 4 338.1 MIP Denisova & Denisov, 2008
Table 9. The values of DO−H of natural phenols
(DO−H(α-tocopherol) = 330.0 kJ/mol), the second column contains the
sites of O−H groups with equireactivity
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
427
As seen from the data in Таb1е 9, all ubiquinols possess
virtually the same dissociation energy оf the 《−H bond, which is
independent оf the length оf а 2-substituent. An average value оf
DO−H is 345.2 ± 0.8 kJ/mol (8 measurements). It should bе borne in
mind that both 《H groups in ubiquinols are involved in hydrogen
bonding with the ortho-methoxy groups. Phenolic groups form very
strong intramolecular hydrogen bonds. For instance, in а phenolic
crown ether (for the structure, see Ref. (Pozdeeva et al., 1989)
the enthalpy оf formation оf such а bond is 21 kJ/mol, whereas the
concentration оf free 《H groups is only 0.1% at 323 К. According to
а theoretical calculation performed bу density functional theory
(Heer et al., 2000) the difference ΔΔG≠ (298 К) for two transition
states for the abstraction оf an H atom bу the methoxyl radica1
from а hydrogen-bonded 《H group оf ubiquinol-0 and from а free 《H
group is 7.5 kJ/mol. Assuming that ΔE(RO2• + ubiquinol) = ΔΔG≠(〈е《•
+ ubiquinol) and using Eqn. (12), we obtain the value of DO−H =
329.0 kJ/mol for а free 《〉 group of ubiquinols, i. e., almost the
same as that for α-tocopherol. In tocopherols, the value DO−H
depends on the number and arrangement of methyl groups in the
aromatic ring (see Таblе 9). At the same time, replacement of
methyl groups bу ethyl, isopropyl, and tert-butyl ones in positions
5 and 7 affects slightly the DO−H values of tocols:
Compound R1 R2 DO−H, kJ/mol 6-Hydroxytocol H H 340.1
6-Hydroxy-5,7-diethyltocol Et Et 333.9
6-Hydroxy-5,7-diisopropyltocol Me2CH Me2CH 335.7
6-Hydroxy-5-isopropyl-7-tert-butyltocol Me2CH Me3C 339.3
Substitution of phytyl (Pht) for the methyl substituent in
position 2 exerts virtually no effect
on the value of DO-H of 6-hydroxychromanes: DO−H(2-Me, 2-Me) −
DO−H(2-Me, 2-Pht) = 0.4 ± 0.7 kJ/mol (7 pairs of compounds from
Таblе 9 were compared). In 6-hydroxy-5,7,8-trimethylchromanes, the
nature of substituents in position 2 virtually has no impact on
the
dissociation energy of the O−H bond: for seven phenols, the
average value is З32.8 ± 2.0 kJ/mol. However, the nature of
5,7,8-substituents in 6-hydroxy-2,2-dimethyl-chromane appreciab1y
influences the value of DO−H altering it in the range 328 to 341
kJ/mol. Substitution of а naphthalene ring for the benzene ring on
going from γ-tocopherol (3) to
6-hydroxy-2,5-dimethyl-2-phytyl-7,8-benzochromane reduces DO−H bу
13 kJ/mol (see Таblе 9). Substitution of S and Se for 《 atoms in
α-tocopherol results in а sma1l decrease in dissociation energy:
DO−H are ЗЗ0.0, 3З4.0 and 335.7 kJ/mol for α-tocopherol, S-, and
Se-analogs, respectively. The presence or the absence of methyl
groups in position 2 in 6-hydroxy-
5,7,8-trimethyl-З,4-dihydrobenzothiopyrans does not affect the
dissociation energy of the 《−〉 bond: DO−H (in kJ/mol) = ЗЗ2.5 (2-〉,
2-〉), ЗЗЗ.9 (2-〉, 2-〈е), З3З.4 (2-〈е, 2-〈е) (see ТаЬ1е 9). The
molecules of chrysin and galangin contain two phenolic groups. One
of them, viz., the 《〉 group in position 5 is linked to the adjacent
carbonyl group bу а hydrogen bond, hence it is the 7-《〉 group that
is the most reactive. As а result, for chrysin and galangin the
number of equireactive 《−〉 bonds (пO-〉 is 1), and DO-H differ
little: З57.1 (chrysin) and 36З.1 (galangin) kJ/mol, respectively.
For morin, D《−〉 of the 《〉 groups in positions 7 and 4’ are
apparently roughly the same and equal to 363.6 kJ/mol (nO−H =
2).
In catechol (1,2-dihydroxybenzene), one hydroxyl group weakens
the adjacent 《−H bond (thus, in pyrogallol DO−H = ЗЗ9.9 kJ/mol,
while in phenol DO−H = З69.0 kJ/mol). A hydrogen bond increases
effective strength of O−H bond roughly bу 10 kJ/mol (for
comparison, in
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
428
quercetin DO-H = З4З.0 kJ/mol and in hesperitin DO-H = З5З.8
kJ/mol); in the latter compound, the peroxyl radical attacks the 《〉
group linked to а methoxy group bу а hydrogen bond. Thus, in
catechol only one 《〉 group reacts with RO2•, the second is inactive
due to the formation of а strong hydrogen bond. An average value of
DO−H in flavanones and flavones is З44.7 ± 2.6 kJ/mol. In
1,2,З-trihydroxybenzenes only one 《−H bond active1y reacts with
RO2•, whereas the other two are involved in hydrogen bonding. For
such phenols а fairly wide range of DO−H values is observed: З47.4
(gallic acid), ЗЗ7.2 ± 2.5 (propyl gallate), З40.9 (myricetin),
З44.6 ((−)-epigallocatechin), З4З.2 (rutin), З45.8 (hesperidin) and
ЗЗ8.7 kJ/mol ((−)-epigallocatechin gallate).
Thus, dissociation energies of the 《−H bond in natural
antioxidants ranges from ЗЗ0 (for α-tocopherol) to З64 kJ/mol (for
morin). These compounds compose а group with very close values of
of DO−H; it includes tocopherols, ubiquinols, flavones, flavanones
and gallates. The
diversity of their structures seems to bе associated with the
peculiarities of the media where they manifest their antioxidant
activity.
3.4 Influence of structure on DO−H of phenols
The most important factor affecting the strength of the 《−H bond
is the stabilization of а phenoxyl radical due to the overlap of
the unpaired electron orbital of the oxygen atom with
the π-electrons of the benzene ring. Тhе stabilization energy
can bе judged bу а comparison of the dissociation energy of the 《−〉
bond in phenol (PhOH) (DO−H = 369 kJ/mol) and in an aliphatic
alcohol ROH (DO−H = 432 kJ/mol) (Luo 2003). The difference is 63
kJ/mol therefore
reactions of peroxyl radicals (DO−H = 365.5 kJ/mol) with most of
phenols, which are
essential for the inhibition of oxidation, are exothermic.
The second factor that influences the dissociation energy of the
《−H bonds of substituted phenols is the inductive effect of alkyl,
in particular, methyl, groups. Below the data are
given that illustrate the role of the inductive effect of methyl
groups on the dissociation
energy of the 《−〉 bond in phenols: ΔD = D(MeC6H4OH) − D(C6H5OH)
kJ/mol (see Tables 2-4, 8).
Substituent ΔD, kJ/mol Substituent ΔD, kJ/mol Substituent ΔD,
kJ/mol 2-Me −9.0 2-Me, 3-Me −13.5 3-Me, 4-Me −14.4 3-Me −3.1 2-Me,
4-Me −8.5 3-Me, 5-Me −4.8 4-Me −7.4 2-Me, 6-Me −15.3 2-Me, 4-Me,
6-Me −13.2
We observe stronger effect on the DO−H for ortho- and
para-methyl groups than that of meta-
methyl group. There is no additivity in action of two or more
methyl groups on DO−H of
substituted phenol. Аnalogous effect is also observed in
tocopherols: the more methyl substituents are present in the
benzene ring of а tocopherol the weaker is its O−H bond.
Phenol nMe DO−H, kJ/mol α-Tocopherol 3 330.0 β-Tocopherol 2
335.5 γ-Tocopherol 2 335.5 δ-Tocopherol 1 361.5
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
429
The third factor is the enhancement of the stabilization of а
phenoxyl radical due to interaction of the p-electrons of the N or
《 atom of amino- and alkoxy- substituent or а hydroxyl group with
the π-electrons of the benzene ring (mesomeric effect). The
magnitude of this effect is clearly seen from the following
comparison:
Substituent of Phenol
ΔD, kJ/mol
Substituent of Phenol
ΔD, kJ/mol
Substituent of Phenol
ΔD, kJ/mol
3-OH −0.6 3-MeO −4.4 3-NH2 −4.7 4-OH −13.9 4-MeO −19.1 4-NH2
−46.8
All these substituents reveal a weak effect on DO−H in
meta-position and very strong in para-position.
The fourth factor is influence of electronegative substituents
that attract the π-electron density of benzene ring and often
increase the dissociation energy of O−H bond. Down are given
examples of such influence.
Substituent of Phenol
ΔD, kJ/mol
Substituent of Phenol
ΔD, kJ/mol
Substituent of Phenol
ΔD, kJ/mol
3-CN −9.4 3-NO2 −2.1 4-COOH 2.7 4-CN 1.2 4-NO2 4.2 4-CF3 9.2
It is seen that influence of substituent depends on position: in
meta-position these substituents decrease DO−H and in para-position
increase DO−H. Quite another effect have haloid substituents (F,
Cl, Br): in meta-position they increase DO−H of phenols and in
ortho- and para-position diminish it (see Table 2). The fifth
factor is the stereoelectronic оnе, which has bееn discussed in
detail by Burton et al. (Burton et al., 1985). The point is that
for bicyclical phenols, such as hydroxychromanes
and hydroxybenzofurans, аn important parameter is the angle θ
between the С−《 bond of the annulated oxygen-containing ring and
the plane of the benzene ring. The smaller this angle the larger
the overlap of the p-electron orbitals of the 《 atom of the pyran
оr furan ring with the π-electcons of the benzene ring and the
higher the stabilization energy of the phenoxyl radical. This is
exemplified bу the data given below:
Phenol
Me
HO
Me
Me
O
Me
MeO
Me
Me
Me
HO
Me
Me Angle θ, deg 6 17 DO−H , kJ/mol 326.4 328.9
The sixth factor is the intramolecular hydrogen bonding. The
value of input of the intramolecular hydrogen bond into DO−H of
ortho-methoxyphenol can be evaluated from
comparison of ΔDO−H estimated by CE and VLPP methods. In the CE
method, the equilibrium
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
430
O + O
HO
Me
OO
O
Me
H
+
proceeds with ortho-methoxyphenol with intramolecular hydrogen
bond and the value of
ΔDO−H = −9.9 kJ/mol (see Table 8) included the input of hydrogen
bond into energy of ortho-methoxyphenoxyl radical stabilization. In
the VLPP method ΔDO−H = −17.6 kJ/mol (see Table 8) was calculated
from comparison of activation energies of decomposition of
anisole
and ortho-methoxyanisole and evidently does not include the
energy of the hydrogen bond.
So, we can evaluate the difference in O−H bond dissociation
energies in ortho-methoxyphenol with and without hydrogen bond as
ΔDO−H…O = −9.9 − (−17.6) = 7.7 kJ/mol. A very close value (ΔDO−H…O
= 7.5 kJ/mоl) gives a quantum chemical calculation of the Gibbs
energy of the transition state for the reaction of the methoxyl
radical with ortho-
methoxyphenol in two distinct states, viz., with а free OH group
and with that bound bу а hydrogen bond (Heer et al., 2000).
The influence of remote hydrogen bond on DO−H value of phenol
was found recently by Foti
et al. (Foti et al., 2010). The comparison of reactivity of 3
substituted phenols in their
reactions with peroxyl (k(RO2•)) and diphenylpycrylhydrazil
(DPPH•) radicals demonstrated
the diversity as the result of formation of remote
intermolecular hydrogen bond.
Phenol
OH
OMe
OMe
OH
O H
O Me
OH
O H
O
Me
k(RO2•), l/mol s (303 K) 4.7 × 105 7.2 × 105 2.5 × 105
k(DPPH•), l/mol s (303 K) 1.8 × 103 4.4 × 103 2.0 × 102 ΔDO−H,
kJ/mol 0.0 −2.5 1.6
One sees that remote hydrogen bonds have appreciable effect on
the phenolic bond
dissociation energy. Intermolecular para-OH…meta-OMe hydrogen
bond weaken, while
meta-OH…para-OMe hydrogen bond strengthen O−H bond dissociation
energy compared with similarly substituted 3,4-dimethoxyphenol.
4. Thermochemistry of hydroperoxides
4.1 Dissociation energies of O−H bonds of hydroperoxides The O−H
bond dissociation energy in tert-butyl hydroperoxide was measured
by Holmes et al. using masspectrometry technique and appearance
energy measurements (Holmes et al., 1991) and was found be equal to
258.6 kJ/mol. All tertiary alkylperoxy radicals has the same
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
431
activity in reactions of hydrogen atom abstraction (Howard,
1972) and hence all tertiary alkylhydroperoxides have the same
DO−H. Secondary alkylperoxy radicals are more active than tertiary
as hydrogen atom acceptors due to the last have lower DO−H (Mill
& Hendry, 1980; Denisov & Afanas’ev, 2005). The difference
in activation energies of reactions:
R’O2 + RH → R’OOH + R
between sec-R’O2 and tert-R’O2 was found be equal to 3.1 ± 1.6
kJ/mol (Denisov & Denisova, 1993). The calculated via MIP
method (Eqn. 13) value of ΔDO−H = DO−H(sec-R’O2) − DO−H(tert-R’O2)
is equal to 6.9 kJ/mol and hence DO−H(sec-ROOH) = DO−H(tert-ROOH) +
6.9 = 365.5 kJ/mol. All primary and secondary alkylhydroperoxide
have
practically the same DO−H (Howard, 1972). In accordance with
these data is equilibrium
constant between secondary and tertiary hydroperoxides and
peroxy radicals (Howard et
al., 1968).
Me
Me
OO +
OOH
Me
Me
OOH +
OO
K
This equilibrium was found be moved to the left and equilibrium
constant K = 0.24 (303 K).
As well as enthalpy of equilibrium ΔH ≅ ΔG = −RTlnK, so ΔH =
ΔDO−H = 3.6 kJ/mol. Mahoney and DaRooge studied the equilibrium
between sec-peroxyl radical and 2,4,6-tri-
tert-butylphenol (Mahoney & DaRooge, 1975).
OO
+ HO
OOH
+ O
The value of DO−H(ROOH) calculated from enthalpy of this
equilibrium was found to cover
the interval 362 ÷ 369 kJ/mol. All data mentioned above are in
agreement with the recommended value DO−H(sec-ROOH) = 365.5 kJ/mol
(Denisov & Denisova, 2000, Denisov
et al., 2003). For the O−H bond dissociation energy of hydrogen
peroxide is recommended the value DO−H(HOOH) = 369.0 kJ/mol (Luo,
2003, Lide, 2004).
Functional groups (Y = OH, >C(O) etc.) in hydroperoxides
influence on their O−H bond dissociation energies. The problem of
estimation of DO−H(YROOH) for such hydroperoxides
was solved recently by using MIP in application to kinetic
experimental data on co-
oxidation of hydrocarbons with compounds YRH including
functional groups (Denisova &
Denisov, 2004). From kinetics of co-oxidation of YRH with
hydrocarbon (RH) ratios of rate
constants kY(YROO + RH)/k(ROO + RH) were calculated and then
estimated the
differences in activation energies: ΔE = E(YROO + RH) − E(ROO +
RH) = RTln(k/kY). These values of ΔE opened the way to estimate the
O−H bond dissociation energies in hydroperoxides with functional
groups (see Eqn. 13 and Table 10).
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
432
ROO−H D, kJ/mol ROO−H D, kJ/mol R1R2CHOO−H 365.5 R1R2R3COO−H
358.6
OH
OO H
362.1
OO
OH
H
358.7
H
OO H
O
369.8
OO
O
H
376.9
R1C(O)OO−H 387.1 OO
O
H
403.9
R1OCH(OO−H)R 367.3 O OO H
367.6
R1R2CHOC(OO−H)R1R2 358.4 R1OCH(OOH)Ph 374.8 R1C(O)CH(OO−H)R
369.8 AcOCH(OOH)Ph 378.0 R1R2NC(OO−H)CHMe 364.1 CCl3CCl2OO−H
413.1
Table 10. The O−H bond dissociation energies in hydroperoxides
with functional groups (Denisova & Denisov, 2004)
There were measured the rate constants for reactions of haloid
substituted methyl and ethyl peroxyl radicals with nonsaturated
fatty acids (Huie & Neta, 1997). These data can be used for
evaluation of DO−H of substituted hydroperoxides in the scope of
MIP. The ratios of rate constants ki(RiO2 + RH)/k1(R1O2 + RH) at T
= 298 K and values of ΔD and D of O−H bonds of ROOH calculated by
Eqns. 10 and 13 are presented in Table 11. The following
parameters
were used for calculation: α = 0.814, bre = 15.21 (kJ/mol)1/2,
A0 = 1.0 × 107 l/mol s (Denisov & Denisova, 2000), Ee1(HO2 +
linoleic acid) = 36.3 kJ/mol and Ee1(CCl3O2 + linolenic acid) =
25.1 kJ/mol.
R1O2 RiO2 RH k1/ki ΔD, kJ/mol D, kJ/mol
HO2 CCl3O2 Linoleic acid 0.012 40.1 409.1
CCl3O2 CF3O2 Linolenic acid 0.16 19.5 428.6
CCl3O2 CBr3O2 Linolenic acid 0.92 0.9 410.0
CCl3O2 CF3CHClO2 Linolenic acid 3.67 −12.7 396.4
Table 11. Dissociation energies of O−H bonds in haloid
substituted hydroperoxides calculated by MIP
Recently these values were used for calculation of enthalpy of
exchange equilibrium reaction (Denisova, 2007):
RO2 + YROOH ROOH + YROO
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
433
where ΔH = DO−H(YROOH) − DO−H(ROOH) in nonpolar solvent. The
reactions and values of ΔH for reactions of exchange between Me3CO2
and YROOH are listed in Table 12.
YROOH D《−〉, kJ/mol ΔH, kJ/mol K (T = 300 K) K (T = 350 K) HOOH
369.0 10.4 1.55 × 10−2 2.80 × 10−2
sec-ROOH 365.5 6.9 6.29 × 10−2 9.34 × 10−2
tert-ROOH 358.6 0.0 1.00 1.00
cyclo-C6H10(OH)OOH 362.1 3.5 2.46 × 10−1 3.00 × 10−1
RPhC(OH)OOH 359.8 1.2 0.62 0.66
ROC(OOH)R 367.3 8.7 3.06 × 10−2 5.03 × 10−2
R2CHOC(OOH)R2 358.4 −0.2 1.08 1.07 × 10−2 ROCH(OOH)Ph 374.8 16.2
1.51 × 10−3 3.82 × 10−3
O OOH
H
367.6 9.0 2.71 × 10−2 4.54 × 10−2
RC(O)OOH 387.1 28.5 1.09 × 10−5 5.58 × 10−5
R3CC(O)OOH 376.9 18.3 6.51 × 10−4 1.86 × 10−3
cyclo-C6H11C(O)OOH 376.9 18.3 6.51 × 10−4 1.86 × 10−3
PhC(O)OOH 403.9 45.3 1.30 × 10−8 1.73 × 10−7
RC(O)CH(OOH)R 369.8 11.2 1.12 × 10−2 2.13 × 10−2
RC(O)CH(OOH)Ph 376.4 17.8 7.06 × 10−4 2.21 × 10−3
CCl3CCl2OOH 413.1 54.5 3.51 × 10−10 7.35 × 10−8
CHCl2CCl2OOH 411.6 53.0 5.92 × 10−10 1.23 × 10−8
Table 12. The values of ΔH for reactions of exchange: Me3CO2 +
YROOH Me3CO2H + YROO (Denisova, 2007)
4.2 Decomposition of α-hydroxyhydroperoxides and
α-hydroxyperoxyl radicals The oxidation of alcohols, their
co-oxidation with other organic compounds, and deep steps
of hydrocarbon oxidation yield α-hydroxyperoxyl radicals
(Denisov & Afanas’ev, 2005). The last participate in the
following reactions:
R1R2C(OH)OO• + R1R2CH(OH) → R1R2C(OH)OOH + R1R2C•(OH)
R1R2C(OH)OO• → R1R2C(O) + HO2• The formed α-hydroxyhydroperoxide
decomposes into carbonyl compound and hydrogen peroxide.
R1R2C(OH)OOH → R1R2C(O) + H2O2
The thermodynamics and kinetic of these reactions were analysed
recently in paper
(Denisov & Denisova, 2006). Hydroxyhydroperoxides are labile
compounds and are not
amenable to thermochemical measurements of their enthalpy of
formation (Denisov et al.,
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
434
2003). Earlier, comparing the enthalpies of formation of
hydroperoxides ROOH with
∆H(RH) and ∆H(ROH), we observed a symbatic change in these
values, namely, the correlations: ∆H(ROOH) = a + ∆H(RH) and
∆H(ROOH) = b + ∆H(ROH) (Denisov & Denisova, 1988). This
regularity was extended to the enthalpy of formation of
α-hydroxyhydroperoxides. The following procedure was used to
estimate
∆H(R1R2C(OH)OOH). First, the difference of the formation
enthalpies of R2CHOOH and R2CH2 was determined, and then the
enthalpy of formation of R
1R2C(OH)OOH was
calculated as the algebraic sum: ∆Hf0
∆Hf0(R1R2C(OH)OOH) = ∆Hf0(R1R2CHOH) + {∆Hf0(R1R2CHOOH) −
∆Hf0(R1R2CH2)} (16)
The results of calculation of the enthalpies of formation for
fourteen α-hydroxyhydroperoxides by Eqn. (16) are given in Table
13. This calculation implies that the
replacement of H by OOH varies the enthalpy of formation of the
corresponding alcohol by
the same value as in the case of this substitution in RH. The
validity of this approach was
qualitatively verified by comparing the enthalpies of two
equilibrium reactions of
cyclohexanone with ROOH and H2O2 (Denisov & Denisova, 2006).
The values of
decomposition enthalpies of α-hydroxyhydroperoxides are listed
in Table 13.
α-Hydroxyhydroperoxide −∆Hf0(R1R2C(O)), kJ/mol
−∆Hf0(R1R2C(OH)OOH), kJ/mol
ΔH, kJ/mol
CH2(OH)OOH 108.8 261.1 15.9
MeCH(OH)OOH 165.7 320.0 17.9
EtCH(OH)OOH 187.4 336.8 13.0
Me2C(OH)OOH 217.1 366.1 12.6
PrCH(OH)OOH 207.5 353.5 9.6
EtMeC(OH)OOH 240.6 385.8 8.8
MePrC(OH)OOH 259.0 401.7 6.3
PhCH(OH)OOH 37.7 190.0 15.9
PhMeC(OH)OOH 86.6 231.8 8.8
cyclo-C6H11CH(OH)OOH 235.1 389.5 18.0
cyclo-C5H8(OH)OOH 192.5 349.2 20.3
cyclo-C6H10(OH)OOH 225.9 377.7 22.4
cyclo-C12H22(OH)OOH 351.5 495.7 7.8
α-Tetralyl-(OH)OOH 90.8 246.0 18.8 Table 13. Enthalpies (ΔH) of
decomposition of α-hydroxyhydroperoxides in nonpolar solvents
According data presented in Table 10 the strength of the OO–H
bond in
α-hydroxycyclohexyl hydroperoxide is equal to 362.1 kJ/mol.
Therefore, using the expression for the strength of the OO–H
bond:
DO−H = ∆Hf0(R2C(OH)OO) + ∆Hf0(H) − ∆Hf0(R2C(OH)OOH) (17)
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
435
and supposing DO−H = 362.1 kJ/mol for all hydroxyhydroperoxides
we obtain the following
thermochemical equation for the enthalpy of formation of the
α-hydroxyperoxyl radical (∆Hf0(H) = 218.0 kJ/mol (Luo, 2005)):
∆Hf0(R2C(OH)OO), kJ/mol = ∆Hf0(R2C(OH)OOH) + 144.1 (18)
The ∆Hf0 (>C(OH)OO) values calculated for decomposition of
fifteen radicals by Eq. (18) are given in Table 14. The enthalpy
(∆H) of decomposition of the α-hydroxyperoxyl radical was
calculated by the Eqn. 19:
∆H(decay), kJ/mol = ∆Hf0(R2C(O)) + ∆Hf0(HO2) − ∆Hf0(R2C(OH)OO)
(19)
where ∆Hf0(HO2• ) = 14.6 kJ/mol (Lide, 2004). The results of
calculation of the enthalpies of degradation of the
α-hydroxyperoxyl radicals are presented in Table 14.
α-Hydroxyperoxyl radical −∆Hf0(>C(OH)OOH)), kJ/mol
−∆Hf0(>C(OH)OO•), kJ/mol
ΔH, kJ/mol
CH2(OH)OO 261.1 117.0 22.8
MeCH(OH)OO 320.0 175.9 24.8
EtCH(OH)OO 336.8 192.7 20.0
Me2C(OH)OO 366.1 222.0 19.5
PrCH(OH)OO 353.5 209.4 16.5
EtMeC(OH)OO 385.8 241.7 15.7
MePrC(OH)OO 401.7 257.6 13.2
Me2CHMeC(OH)OO 401.7 257.6 9.9
PhCH(OH)OO 190.0 45.9 22.8
PhMeC(OH)OO 231.8 87.7 15.7
cyclo-C6H11CH(OH)OO 389.5 245.4 25.0
cyclo-C5H8(OH)OO 349.2 205.1 27.2
cyclo-C6H10(OH)OO 377.7 233.4 22.4
cyclo-C12H22(OH)OO 495.7 351.6 15.0
α-Tetralyl-(OH)OO 246.0 101.9 25.7 Table 14. Enthalpies of
decomposition of α-hydroxyperoxyl radicals
4.3 Enthalpies of reactions of peroxyl radicals with phenols
As was written earlier, the reaction of peroxyl radicals with
phenols is the main reaction of action of phenols as antioxidants.
The enthalpy of this reaction is equal to difference of bond
dissociation energies of two O−H bonds:
ΔH = DO−H(ArOH) − DO−H(ROOH) . (20)
The values of ΔH calculated for 108 reactions of different RiO2
with phenols (ArjOH) are presented in Table 15. It is seen from
Table 15 that enthalpy of reaction strongly depends on DO−H(ArOH)
as well as on DO−H(ROOH).
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
436
ΔH, kJ/mol ArjOH/RiO2 tert-ROO sec-ROO HO2 AcCH(OO)Me AcOO
PhC(O)OO
PhOH 10.4 3.5 0.0 1.7 −18.1 −34.9 4-Me-C6H4OH 3.0 −3.9 −7.4 −5.7
−25.5 −42.3 4-OMe-C6H4OH −8.7 −15.6 −19.1 −17.4 −37.2 −54.0
4-OH-C6H4OH −3.5 −10.4 −13.9 −12.2 −32.0 −48.8 4-NH2-C6H4OH −36.4
−43.3 −46.8 −45.1 −64.9 −81.7 4-COMe-C6H4OH 12.9 6.0 2.5 4.2 −15.6
−32.4 2,4-(Me)2-C6H3OH 1.9 −5.0 −8.5 −6.8 −26.6 −43.4 2,6
-(Me)2-C6H3OH −4.0 −10.9 −14.4 −12.7 −32.5 −49.3 Ionol −15.6 −22.5
−26.0 −24.3 −44.1 −60.9 α-Tocopherol −28.6 −35.5 −39.0 −37.3 −57.1
−73.9 β-Tocopherol −23.3 −30.2 −33.7 −32.0 −51.8 −68.6 δ-Tocopherol
−17.1 −24.0 −27.5 −25.8 −45.6 −62.4 Ubiquinol-0 −13.3 −20.2 −23.7
−22.0 −41.8 −58.6 Quercetin −15.6 −22.5 −26.0 −24.3 −44.1 −60.9
Chrysin −1.5 −8.4 −11.9 −10.2 −30.0 −46.8 Morin 5.0 −1.9 −5.4 −3.7
−23.5 −40.3 Campherol −9.7 −16.6 −20.1 −18.2 −38.2 −55.0 Myricetin
−17.7 −24.6 −28.1 −26.4 −46.2 −63.0
Table 15. Enthalpies (kJ/mol) of reactions RiO2• + ArjOH → RiOOH
+ ArjO• (Eqn. 20)
5. References
Angel, L. & Ervin, K. (2004). Competitive Threshold
Collision-Induced Dissociation: Gas-Phase Acidity and O−H Bond
Dissociation Enthalpy of Phenol. J. Phys. Chem. A, Vol. 108, No.
40, 8346-8352, ISSN 1089-5639
Arnett, E., Amarnath, K., Harvey, N. & Venimadhavan, S.
(1990). Heterolysis and Homolysis Energies of Some Carbon-Oxygen
Bonds. J. Am. Chem. Soc., Vol. 112, No. 20, 7346-7353, ISSN
0002-7863
Belyakov, V., Shanina, E., Roginsky, V. & Miller, V. (1975).
O−H Bond Energies and the Inhibiting Action of Sterically Hindered
Phenols. Izv. Akad. Nauk SSSR, Ser. Khim. (Russian), No. 12,
2685-2691, ISSN 0002-3353
Bordwell, F. & Bausch, M. (1986).
Acidity-Oxidation-Potential (AOP) Values as Estimates of Relative
Bond Dissociation Energies and Radical Stabilities in Dimethyl
Sulfoxide Solution. J. Am. Chem. Soc., Vol. 108, No. 8, 1979-1985,
ISSN 0002-7863
Bordwell, F. & Cheng, J.-P. (1991). Substituent Effects on
the Stabilities of Phenoxyl Radicals and the Acidities of Phenoxyl
Radical Cations. J. Am. Chem. Soc., Vol. 113, No. 5, 1736-1743,
ISSN 0002-7863
Bordwell, F., Cheng, J.-P., Ji, G.-Z., Satish, A. & Zhang,
X. (1991). Bond Dissociation energies in DMSO Related to the Gas
Phase. J. Am. Chem. Soc., Vol. 113, No. 26, 9790-9795, ISSN
0002-7863
Bordwell, F. & Liu, W.-Z. (1996). Equilibrium Acidities and
Homolytic Bond Dissociation Energies of N−H and/or O−H Bonds in
N-Phenylhydroxylamine and Its Derivatives. J. Am. Chem. Soc., Vol.
118, No. 37, 8777-8781, ISSN 0002-7863
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
437
Burton, G., Doba, T., Gabe, E., Hughes, L., Lee, F., Prasad, L.
& Ingold, K. (1985). Autoxidation of Biological Molecules. 4.
Maximizing the Antioxidant Activity of Phenols. J. Am. Chem. Soc.,
Vol. 107, No. 24, 7053-7065, ISSN 0002-7863
Burton, G. & Ingold, K. (1986). Vitamin E: Application of
the Principles of Physical Organic Chemistry to the Exploration of
Its Structure and Function. Acc. Chem. Res., Vol. 19, No. 7,
194-201, ISSN 0001-4842
Denisov, E. (1995a). A new semiempirical method of estimation of
activity and bond dissociation energies of antioxidants. Polymer
Degradation and Stability, Vol. 49, No. 1, 71-75, ISSN
0141-3910
Denisov, E. (1995b). Evaluation of the dissociation energies of
the O−H bonds of phenols on the basis of kinetic measurements.
Russ. J. Phys. Chem., Vol. 69, No. 4, 563-574, ISSN 0036-0244
Denisov, E. (1997). New empirical models of radical abstraction
reactions. Russ. Chem. Rev., Vol. 66, No. 10, 859-876, ISSN
0036-021X
Denisov, E. (1999). Models for Abstraction and Addition
Reactions of Free Radicals, In: General Aspects of the Chemistry of
Radicals. Alfassi, Z. (Ed.), 79-137, Wiley and Sons, ISBN
0-471-98760-3, Chichester, UK
Denisov, E. & Afanas’ev, I. (2005). Oxidation and
Antioxidants in Organic Chemistry and Biology, Taylor and Francis,
ISBN 0-8247-5356-9, Boca Raton, FL
Denisov, E. & Azatyan, V. (2000). Inhibition of Chain
Reaction, Gordon and Breach Science Publishers, ISBN 90-6994-002-7,
London
Denisov, E. & Denisova, T. (1988). The Enthalpies of
Formation of Peroxy Radicals and
Dissociation Energies, of C−O and O−O Bonds in Peroxy Radicals
and Hydroperoxides. Zh. Fiz. Khim. (Russian), Vol. 62, No. 2,
304-309, ISSN 0044-4537
Denisov, E. & Denisova, T. (1993). Kinetic Parameters of the
Reactions RO2• + RH in the
Framework of the Parabolic Model of Transition State. Kinet.
Сatal., Vol. 34, No. 2, 173-179, ISSN 0023-1584
Denisov, E. & Denisova, T. (2000). Handbook of Antioxidants.
CRC Press, ISBN 0-8493-9004-4, Boca Raton, FL
Denisov, E. & Denisova, T. (2006). Kinetics and
Thermodynamics of Formation and
Degradation of α-Hydroperoxy Radicals. Pet. Chem., Vol. 46, No.
6, 373-383, ISSN 0965-5441
Denisov, E. & Denisova, T. (2009). The Reactivity of Natural
Phenols. Russ. Chem. Rev., Vol. 78, No. 11, 1047-1073, ISSN
0036-021X
Denisov, E., Denisova, T. & Pokidova, T. (2003). Handbook of
Free Radical Initiators. John Wiley & Sons, ISBN 0-471-20753-5,
Hoboken, NJ
Denisov, E. & Khudyakov, I. (1987). Mechanisms of action and
reactivities of the free radicals of inhibitors. Chem. Rev., Vol.
87, No. 6, 1313-1357, ISSN 0009-2665
Denisov, E. & Kovalev, G. (1983). Okislenie i Stabilizatsiya
Reactivnykh Topliv (Oxidation and Stabilization of Jet Fuels),
Khimiya Publishers, Moscow (Russian)
Denisov, E. & Tumanov, V. (2005). Estimation of the bond
dissociation energies from the kinetic characteristics of
liquid-phase radical reactions. Russ. Chem. Rev., Vol. 74, No. 9,
825-858, ISSN 0036-021X
Denisova, T. (2007). Kinetics and Thermodynamics of the Exchange
Reactions of Peroxy radicals with Hydroperoxides. Kinet. Сatal.
(Engl. Transl.), Vol. 48, No. 5, 609-614, ISSN 0023-1584
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Science
438
Denisova, T. & Denisov, E. (2004). Estimation of the O−H
Bond Dissociation Energy from Kinetic Data for Hydroperoxides with
Functional Group. Pet. Chem., Vol. 44, No. 4, 250-255, ISSN
0965-5441
Denisova, T. & Denisov, E. (2008). Dissociation energies of
O−H bonds in natural antioxidants. Russ. Chem. Bull., Int. Ed.,
Vol. 57, No. 9, 1858-1866, ISSN 1066-5285
Emanuel, N., Denisov, E. & Maizus, Z. (1967). Liquid-Phase
Oxidation of Hydrocarbons, Plenum Press, Number 66-12888, New
York
Emanuel, N. & Lyaskovskaya, Yu. (1961). Tormozhenie
Protsessov Okisleniya Zhirov. (Inhibition of Fat Oxidation),
Pische-promizdat, Moscow (Russian)
Foti, M., Amorati, R., Pedulli, G. F., Daquino, C., Pratt, D.
& Ingold, K. (2010). Influence of “Remote” Intramolecular
Hydrogen Bonds on the Stabilities of Phenoxyl Radicals and Benzyl
Cations. J. Org. Chem., Vol. 75, No. 13, 4434-4440, ISSN
0022-3263
Golden, D., Spokes, G. & Benson, S. (1973). Very
Low-Pressure Pyrolysis (VLPP); A Versatile Kinetic Tool. Angew.
Chem. Int. Ed. Egl., Vol. 12, No. 7, 534-546, ISSN 0570-0833
Grabowski, J., Simon, J. & Peters, K. (1984). Heat of
Formation of Diphenylcyclopropenone
by Photoacoustic Calorimetry. J. Am. Chem. Soc., Vol. 106, No.
16, 4615-4616, ISSN
0002-7863
Hamid, S. (Ed.), (2000). Handbook of Polymer Degradation, Marcel
Dekker, ISBN 0-8247-0324-3,
New York
de Heer, M., Mulder, P., Korth, H.-G., Ingold, K. & Lusztyk,
J. (2000). Hydrogen Atom
Abstraction Kinetics from Intramolecularly Hydrogen Bonded
Ubiquinol-0 and
other (Poly)methoxy Phenols. J. Am. Chem. Soc., Vol. 122, No.
10, 2355-2360, ISSN
0002-7863
Holmes, J., Lossing, F. & Mayer, P. (1991). Heats of
Formation of Oxygen Containing
Organic Free Radicals from Apperange Energy Measurements. J. Am.
Chem. Soc.,
Vol. 113, No. 26, 9723-9728, ISSN 0002-7863
Howard, J. (1972). Absolute Rate Constants for Reactions of Oxyl
Radicals, In: Advances in
Free Radical Chemistry. Williams, G. (Ed.), Vol. 4, 49-173,
Logos Press, ISBN
0236176625, London
Howard, J. & Ingold, K. (1965). The kinetics of inhibited
oxidation of tetralin. Can J. Chem.,
Vol. 43, No. 10, 2724-2728, ISSN 0008-4042
Howard, J., Schwalm, W. & Ingold, K. (1968). Absolute Rate
Constants for Hydrocarbon
Autoxidation. VII. Reactivities of Peroxy Radicals Toward
Hydrocarbons and
Hydroperoxides. In: Oxidation of Organic Compounds-1; Adv. Chem.
Ser. 75, Gould, R.
(Ed), Proceedings of the International Oxidation Symposium, Vol.
75, pp. 6-23, LCCC
967-7520, Stanford Research Institute, San Francisco, Calif.
Aug. 28 – Sept. 1, 1967,
American Chemical Society, Washinton
Huie, R. E. & Neta, P. (1997). Kinetic Studies of Organic
Peroxyl Radicals in Aqueous
Solutions and Mixed Solvents, In: Peroxyl Radicals. Alfassi, Z.
B. (Ed.), 235-281,
Wiley and Sons, ISBN-10: 0471970654, ISBN-13: 9780471970651,
Chichester, UK
Jackson, R. & Hosseini, K. (1992). Phenol-Phenoxyl Radical
Equilibria by Electron Spin
Resonance: are Radicals Derived from Tocopherol and Analogues
Exceptionally
Stabilized? J. Chem. Soc., Chem. Commun., No. 13, 967-968, ISSN
0022-4936
Kuliev, A. (1972). Khimiya i Tekhnologiya Prisadok k Maslam i
Toplivam (Chemistry and
Technology of Additives to Oils and Fuels), Khimiya Publishers,
3-14-7-69-72, Moscow
(Russian)
www.intechopen.com
-
Dissociation Energies of O−H Bonds of Phenols and
Hydroperoxides
439
Laarhoven, L., Mulder, P. & Wayner, D. (1999). Determination
of Bond Dissociation
Enthalpies in Solution by Photoacoustic Calorimetry. Acc. Chem.
Res., Vol. 32, No. 4,
342-349, ISSN 0001-4842
Lide, D. (Ed.), (2004-2005). Handbook of Chemistry and Physics.
85 Edition. CRC Press, ISBN 0-
8493-0485-7, Boca Raton, FL
Lind, J., Shen, X. Eriksen, T. & Merenyi, G. (1990). The One
Electron Reduction Potencial of
4-Substituted Phenoxyl Radicals in Water. J. Am. Chem. Soc.,
Vol. 112, No. 2, 479-
482, ISSN 0002-7863
Lucarini, M., Mugnaini, V. & Pedulli, G. F. (2002). Bond
Dissociation Enthalpies of Polyphenols: the Importance of
Cooperative Effects. J. Org. Chem., Vol. 67, No. 3, 928-931, ISSN
0022-3263
Lucarini, M. & Pedulli, G. F. (2010). Free radical
intermediates in the inhibition of the
autoxidation reaction. Chem. Soc. Rev., Vol. 39, 2106-2119, ISSN
0306-0012
Lucarini, M., Pedulli, G. F. & Cipollone, M. (1994). Bond
Dissociation Enthalpy of α-Tocopherol and Other Phenolic
Antioxidants. J. Org. Chem., Vol. 59, No. 17, 5063-5070, ISSN
0022-3263
Lucarini, M., Pedrielli, P., Pedulli, G. F., Cabiddu, S. &
Fattuoni, C. (1996). Bond Dissociation Energies of O−H Bonds in
Substituted Phenols from Equilibration Studies. J. Org. Chem., Vol.
61, No. 26, 9259-9263, ISSN 0022-3263
Luo, Y-R. (2003). Handbook of Bond Dissociation Energies in
Organic Compounds, CRC Press, ISBN 0-8493-1589-1, Boca Raton,
FL
Luzhkov, V. (2005). Mechanisms of antioxidant activity: The DFT
study of hydrogen abstraction from phenol and toluene by the
hydroperoxyl radical. Chem. Phys., Vol. 314, No. 1-3, 211-217, ISSN
0301-0104
Mahoney, L. & DaRooge, M. (1975). The Kinetic Behavior and
Thermochemical Properties of Phenoxy Radicals. J. Am. Chem. Soc.,
Vol. 97, No. 16, 4722-4731, ISSN 0002-7863
Mahoney, L. Ferris, F. & DaRooge, M. (1969). Calorimetric
Study of the 2,4,6-Tri-t-butylphenoxy Radical in Solution. J. Am.
Chem. Soc., Vol. 91, No. 14, 3883-3889, ISSN 0002-7863
Mill, T. & Hendry, D. (1980). Kinetics and Mechanisms of
Free Radical Oxidation of Alkanes and Olefins in the Liquid Phase,
In: Comprehensive Chemical Kinetics. Liquid-Phase Oxidation,
Bamford, C. & Tipper, C. (Eds.), Vol. 16, 1-87, Elsevier, ISBN
0-444-41860-1, Amsterdam
Mogilevich, M. & Pliss, E. (1990). Okislenie i
Okislitel’naya Polimerizatsiya Nepredel’nykh Soedinenii (Oxidation
and Oxidative Polymerisation of Unsaturated Compounds), Khimiya
Publishers, ISBN 5-7245-0564-9, Moscow (Russian)
Mulder, P., Korth, H-G., Pratt, D., DiLabio, G., Valgimigly, L.,
Pedulli, G.F. & Ingold, K. (2005). Critical Re-evaluation of
the O−H Bond Dissociation Enthalpy in Phenol. J. Phys. Chem. A,
Vol. 109, No. 11, 2647-2655, ISSN 1089-5639
Pratt, D., de Heer, M., Mulder, P. & Ingold, K. (2001).
Oxygen-Carbon Bond Dissociation Enthalpies of Benzyl Phenyl Ethers
and Anisoles. An Example of Temperature Dependent Substituent
Effects. J. Am. Chem. Soc., Vol. 123, No. 23, 5518-5526, ISSN
0002-7863
Pospisil, J. & Klemchuk, P. (Eds.), (1990). Oxidation
Inhibition in Organic Materials, Vol. 1-2, CRC Press, ISBN-10:
08493-4767X ISBN-13: 9780849347672, Boca Raton, FL
www.intechopen.com
-
Application of Thermodynamics to Biological and Materials
Scie